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%yield = 6.1 tons × 100 = 64%<br />
9.6tons<br />
Discussion<br />
Due to chemical equilibrium or the mass action law, the limiting reagent may not be completely<br />
consumed. Thus, a lower yield is expected in some cases. Losses during the recovery process of the<br />
product will cause an even lower actual yield.<br />
Example 2<br />
A solution containing silver ion, Ag + , has been treated with excess of chloride ions Cl − . When dried,<br />
0.1234 g of AgCl was recovered. Assuming the percentage yield to be 98.7%, how many grams of<br />
silver ions were present in the solution?<br />
Hint:<br />
The reaction and relative masses of reagents and product are:<br />
The calculation,<br />
Ag + (aq) + Cl − (aq) → AgCl(s)<br />
107.868 + 35.453 = 143.321<br />
0.1234 g AgCl ×107.868 g Ag + =0.09287 g Ag +<br />
143.321g AgCl<br />
shows that 0.1234 g dry AgCl comes from 0.09287g Ag + ions. Since the actual yield is only 98.7%,<br />
the actual amount of Ag + ions present is therefore<br />
0.09287 g Ag + = 0.09409 g Ag +<br />
0.987<br />
Discussion<br />
One can also calculate the theoretical yield of AgCl from the percentage yield of 98.7% to be<br />
0.1234 g AgCl =0.1250 g AgCl<br />
0.987<br />
From 0.1250 g AgCl, the amount of Ag + present is also 0.09409 g.<br />
Stoichiometry - A Review<br />
Skills Taught<br />
<br />
<br />
<br />
<br />
<br />
<br />
<br />
evaluate molecular weight for a given formula<br />
evaluate weight (mass) percentages of elements for a given formula<br />
evaluate amounts (in mass and mole units) produced in a chemical reaction from given<br />
conditions<br />
classify reactions by types: combination, combustion, displacement, formation, etc<br />
determine the chemical formula when weight percentages are given and then evaluate the<br />
mole percentages of elements in the formula<br />
determine the chemical formula when weight percentages are given and molecular weight is<br />
known<br />
determine the amount produced, the actual yield, and other stoichiometry quantities for a given<br />
reaction